A 0.727-g sample of the sugar D-ribose (C5H10O5) was placed in a calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K. In a separate experiment in the same calorimeter, the combustion of 0.825 g of benzoic acid (Ucomb. = 3251 kJ/mol), gave a temperature rise of 1.904 K. Calculate following quantities. (a) calorimeter constant. (b) standard internal energy of combustion of D-ribose (c) standard enthalpy of combustion of D-ribose (d) standard enthalpy of formation of D-ribose.
A 0.727-g sample of the sugar D-ribose (C5H10O5) was placed in a calorimeter and then ignited...
31. A sample of the sugar D-ribose of mass 0.727 g was placed in a calorimeter and then ignited in the presence of excess oxygen. The temperature rose by 0.910 K.. In a separate experiment in the same calorimeter, the combustion of 0.917 g of benzoic acid, for which the internal energy of combustion is - 3226 kJ mol-1, gave a temperature rise of 1.940 K. Calculate the enthalpy of formation of D-ribose. 33. The mean bond enthalpies of C-C,...
Bomb calorimetry is a technique used to determine the enthalpy of combustion, usually in O2, of a chemical species. A known amount of compound is placed inside a fixed volume container that is, in turn, filled with oxygen at a high enough pressure to ensure complete combustion. The fixed-volume container (the 'bomb') is then inserted into a bucket containing a precisely known volume of water. The oxygen and compound are ignited, and the temperature change in the water is recorded....
A sample of solid bianthracene (C28H18) that weighs 0.5275 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.170 °C. The heat capacity of the calorimeter and its contents is known to be 9.520×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Based on this experiment: (b) Assuming that H° is approximately equal...
A sample of solid pyrene (C16H10) that weighs 0.5063 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.130 °C. The heat capacity of the calorimeter and its contents is known to be 9.233×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or...
A 0.1785 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/C. If the temperature rise of the calorimeter with water was 1.25*C, calculate the enthalpy of combustion(in kJ/mol) of magnesium. Mg(s) + 1/2O2(g) -> MgO(s) Write answer to three significant figures. Numeric Response
A sample of solid 1,9-nonanediol (C9H20O2) that weighs 0.5724 g is burned in an excess of oxygen to CO2(g) and H2O(l) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.210 °C. The heat capacity of the calorimeter and its contents is known to be 9.268×10^3 J K^-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Please specify states such as (aq) or (s). ____+____--->____+____ Based on...
A sample of solid 1,2-benzenediol (C6H6O2) that weighs 0.8129 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.270 °C. The heat capacity of the calorimeter and its contents is known to be 9.301×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction.Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s)....
A sample of solid diphenyl phthalate (C20H14O4) that weighs 0.6847 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.110 °C. The heat capacity of the calorimeter and its contents is known to be 9.580×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq)...
A 1.0422 g sample of powdered aluminum is burned in a constant volume bomb calorimeter containing excess oxygen to form Al_2 O_3 (s) The calorimeter has a heat capacity of 8.775 kJ degree C^-1. The temperature of the calorimeter increases by 3.680 degree C. Determine the molar internal energy of combustion delta U and the molar enthalpy of combustion delta H for aluminum at 25 degree C. 4 Al (s) + 3 O_2 (g) middot 2 Al_2 O_3 (s)
I need c,d,e, and f please. 2.00 g of Benzoic Acid arc burned in a bomb calorimeter, and the temperature increases from 17.84 degree C to 23.34 degree C. What is the heat capacity of the calorimeter? You burn 4.08 g of Arginine in the bomb calorimeter. The temperature increases from 17.49 degree C to 23.83 degree C. Determine the enthalpy of combusion and the enthalpy of formation of Arginine. Arginine has a standard molar entropy of 250.G J/mol K....